Chapter 10 - Reaction Rates and Equilibrium Flashcards
How do you calculate the rate of a reaction?
Rate = change in concentration / time
(units = mol dm^-3 s^-1)
What factors change the rate of a chemical reaction?
-Concentration
-Temperature
-Surface area
-Use of catalyst
What is the collision theory?
The collision theory states that in order for a reaction to take place, two particles must collide with enough force
What makes a collision effective?
-Correct orientation
-Enough energy to overcome the activation energy
What effect does concentration have on rate of reaction?
When the concentration of reactants is increased, the rate of reaction will increase. This is because there are more particles in the same volume so the particles are closer together and collide more frequently, so there will be more successful collisions per unit time and an increased rate of reaction
How does increasing pressure of a gas affect rate of reaction?
The rate of reaction will also increase as the same number of gas molecules occupy a smaller volume, so they are closer together and collide more frequently, so there are more successful collisions
How do you measure the progress of a reaction?
-Measure decrease in concentration of reactants
-Measure increase in concentration of products
What is a catalyst?
A substance that increases the rate of reaction without being used up. it does this by lowering the activation energy
What is a homogeneous catalyst?
A catalyst that has the same physical state as the reactants. The catalyst reacts with the reactants to form an intermediate product, this then breaks down to form the final product
What is a heterogeneous catalyst?
A catalyst that is in a different physical state than the reactants
Why are catalysts often used in industry?
They reduce the temperature needed for the process and the energy required, this means less electricity / fossil fuels are used which can cut costs and increase profitability
What does a Boltzmann distribution curve look like?
How does the Boltzmann distribution curve change at higher temperatures?
-More molecules have energy greater than or equal to the activation energy
-Therefore more of the collisions will lead to a reaction, so the rate of reaction increases
-Collisions are also more frequent as the molecules are moving faster
How does the Boltzmann distribution curve change with the use of a catalyst?
-A catalyst lowers the activation energy by providing an alternative route for the reaction so that a greater proportion on the molecules exceeds the lower activation energy
What is dynamic equalibrium?
The equilibrium that exists in a closed system when the rate of the forward reaction is equal to the rate of the reverse reaction and concentrations do not change